Problem: The decomposition of HI(g) is represented by the equation2HI(g) ⇌ H2(g) + I2(g)The following experiment was devised to determine the equilibrium constant of the reaction. HI (g) is introduced into five identical 400-cm3 glass bulbs, and the five bulbs are maintained at 623 K. The amount of I2 produced over time is measured by opening each bulb and titrating the contents with 0.0150 M Na2S2O3 (aq). The reaction of I2 with the titrant isI2 + 2Na2S2O3 ⇌ Na2S4O6 + 2NaIData for the experiment are provided in this table.What is the value of Kc for the decomposition of HI at 623 K?

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FREE Expert Solution

We’re asked to determine the equilibrium constant K_c for the decomposition of HI at 623 K, based on the titration data.

In equilibrium, the amount of I₂ produced is the same amount that was titrated by Na₂S₂O₃.

Titration reaction occurs in a 1:2 mole ratio, where 1 mole of I₂ reacts with 2 moles of Na₂S₂O₃.

This way, we can determine the amount of I₂ in the decomposition reaction.

To determine Kc, we do the following steps:

Step 1: Calculate the moles of I₂ in equilibrium, from the volume of titrant used.